Molar volume = total volume / number of moles = 60 L / 3 moles = 20 L/mole.

Volume per mole = total volume / number of moles = 60 L / 3 moles = 20 L/mole.

The balanced equation is 4Al + 3O2 → 2Al2O3, which shows that 4 moles of Al produce 2 moles of Al2O3.

Molality (m) = moles of solute / kg of solvent = 4 moles / 2 kg = 2 m.

Molality (m) = moles of solute / kg of solvent = 5 moles / 1 kg = 5 m.

Molality (m) = moles of solute / kg of solvent = 5 moles / 3 kg = 1.67 m.

Each mole of NaCl dissociates into 1 mole of Na+ ions. Therefore, 5 moles of NaCl will produce 5 moles of Na+ ions.

Moles of KCl = 50 g / 74.5 g/mol = 0.672 moles. Molarity = 0.672 moles / 0.25 L = 2.688 M.

Mass/volume percent = (mass of solute / volume of solution) * 100 = (50 g / 200 mL) * 100 = 25%.

Moles of NaCl = 50 g / 58.5 g/mol = 0.854 moles. Molarity = 0.854 moles / 1 L = 0.854 M.

Moles of NaOH = 50 g / 40 g/mol = 1.25 moles. Molarity = 1.25 moles / 1 L = 1.25 M.

HCl and NaOH neutralize each other, resulting in a neutral solution with pH = 7.

Subtracting 4x from both sides gives 3x - 3 = 6, then adding 3 gives 3x = 9, leading to x = 3.

Dividing both sides by 7 gives x = 3.

In this case, the reaction force at each support is half the load applied at the center.

The horizontal component is calculated as 10 N * cos(30°) = 8.66 N.

A ΔG of +5 kJ/mol indicates that the reaction is non-spontaneous.

ΔG = ΔH - TΔS = 100 kJ - 298 K * (-0.2 kJ/K) = 100 kJ + 59.6 kJ = 159.6 kJ.

Using Raoult's Law, the mole fraction of the solvent can be calculated as 80 mmHg / 100 mmHg = 0.8, which corresponds to a mole fraction of 0.75 for the solvent.

The quantum numbers correspond to the 2s orbital, where l=0 indicates an s orbital.

The spin quantum number can be either +1/2 or -1/2, so both values are possible.

For l=1, the electron occupies a p orbital.

For l=1, the orbital is a p orbital.

For l=0, m_l can only be 0.

For l=2, m_l can take values -2, -1, 0, 1, 2. Therefore, all of the options are valid.

For l=2, the orbital type is d.

According to the Arrhenius equation, an increase in activation energy results in a decrease in the rate constant k.

The azimuthal quantum number l = 1 corresponds to p orbitals, which have a dumbbell shape.

According to Le Chatelier's principle, increasing the concentration of reactants will shift the equilibrium position to the right, favoring the formation of products.

If the enthalpy of a system increases, the process is considered endothermic.